# Percent Yield Theoretical Yield Actual Yield

Percent Yield Theoretical Yield Actual Yield Theoretical Yield The maximum amount of product that can be formed from given

amounts of reactants The amount you should get in a perfect world Use equation and stoichiometry to calculate this amount Actual Yield

The amount of product that actually forms when a reaction is carried out in the lab Percent Yield A measure of the efficiency of a

reaction carried out in the lab The ratio of the actual yield to the theoretical yield Percent yield = actual yield theoretical yield

x 100% Percent yield should not be greater than 100% Often less than 100% Rxns. dont always go to

completion Some product can be lost during filtering or transferring Reactants or products not measured carefully When 84.8 g of iron(III) oxide reacts with an

excess of carbon monoxide, iron is produced. Fe2O3(s) + 3CO(g) 2Fe(s) + 3CO2(g) What is the theoretical yield of iron? When 5.00 g of copper reacts with excess silver nitrate, silver metal and copper(II) nitrate are produced. What is the theoretical yield of

silver in this reaction? If 50.0 g of silicon dioxide is heated with an excess of carbon, 27.9 g of silicon carbide is produced. SiO2(g) + 3C(s) SiC(s) + 2CO(g) What is the percent yield of this reaction?

If 15.0 g of nitrogen reacts with 15.0 g of hydrogen, 10.5 g of ammonia is produced. What is the percent yield of this reaction?

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